It is not practicable to measure the intercept directly at 1/T=0, so calculate ln A from the measured slope and the coordinates of any point on the graph. Compare your values of E and A with those obtained by previous students, namely E = 52 kJ mol-1 and A = ~107 dm3 mol-1 s-1
For E = 45.3953 kJ mol-1
equation: y = -5460.1x + 10.272
At 273K, 301K and 308K, I calculate the A, but it's ~3 x 10-3 dm3 mol-1 s-1


It is not practicable to measure the intercept directly at 1/T=0, so calculate ln A from the meas...
Temp
k
0 °C
6.6667 x 10-5
28°C
2.0560 x 10-4
35°C
9.6155 x 10-4
It is not practicable to measure the intercept directly at 1/T-0, so calculate In A from the measured slope and the coordinates of any point on the graph. Compare your values of E and A with those obtained by previous students, namely E-52 kJ mol 1 and A- ~10 dm mol-1 s1 For E-45.3953 kJ mole equation: y -5460.1 x + 10.272- At 273K, 301K...
Table 3: Experimental Data for Part 2: Determination of Activation Energy k Time* T* [1] [S,0,?] Rate (M/s) (s) (C) (M) (M) Run 3 153 20.5 .0208 .0416 4.03*10^-6 4.65*10^-3 (Room T) Run 6 198 9 .0208 .0416 3.15*10^-6 3.64*10^-3 (Cool) Run 7 112 31 .0208 .0416 5.58*10^-6 6.45*10^-3 (Warm) Run 8 40 51 .0208 .0416 1.56*10^-5 1.80*10^-2 (Warmer) 1/T (1/K) In k Run 3 1/293.5 -5.37 Run 6 1/282 -5.62 Run 7 1/304 -5.044 Run 8 1/324 -4.02 20....
rates of chemical reactions
Plz help!! how do I find specific rate constant k, 1/T, In
K
thank you
Rates of Chemical Reactions: Report Form Rate Law Summary: (a) From your measurements, what are the reaction orders with respect to each of the three reactants H;O; HOO (b) What is the rate expression (rate law) for the uncatalyzed reaction? Rate = K LT-] [H202) (c) What is the total reaction order? 2 3. Effect of Temperature on the Reaction Rate...